13. A 60.0 g block of iron that has an initial temperature of 250. °C and 60.0 g block of gold that has an initial temperature of 45.0 °C are brought into contact with one another. Assuming no heat is lost to the surroundings, what will be the temperature when the two metals reach thermal equilibrium? The specific heat capacity of iron = 0.449 J/g C and gold 0.128 J/g* C. %3D

13. A 60.0 g block of iron that has an initial temperature of 250. °C and 60.0 g block of gold that has an initial temperature of 45.0 °C are brought into contact with one another. Assuming no heat is lost to the surroundings, what will be the temperature when the two metals reach thermal equilibrium? The specific heat capacity of iron = 0.449 J/g C and gold 0.128 J/g* C. %3D

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

#18
12. When 30.0 mL of 1.00 M HCl(aq) and 45.0 mL of 1.00 M NaOH(aq), both at 21.0 °C, are added to a coffee cup calorimeter, the temperature of the mixture reaches a maximum of 24.0° What is the amount of heat produced by this reaction? The mixture has a specific heat of 4.184 J/g °C and density of 1g/mL. Show work and write your answers in 4 significant figures. Box in your final answer. HCl(aq) + NaOH(aq) --> NaCl(aq) + H₂O(1)
A 22.0 g piece of metal is heated to 100.0°C and placed in 75.0g of water at 25.0°C. if the final temperature of the metal and water is 27.8°C, what is the specific heat capacity of the metal in J/g°C? The specific heat capacity of water is 4.184 J/g°C. а. 0.038 b. 0.16 c. 0.55 d. 5.0 a
6. A substance increases in temperature by 55°C when a 98 g sample of it absorbs 80000 J of heat. What is the specific heat capacity of the substance?
17. An ice cube is placed in a sealed insulated container of hot water at 80°C. After five minutes, the ice cube disappears. Ice Cube Heat ener Hot Water 5 min. Water Which best describes the change that took place inside the container? The total heat energy in the container was reduced by the ice cube. The hot water lost the same amount of heat energy as the ice cube gained. in the hot water was reduced by kinetic energy in the ice cube. O Heat energy in the ice cube was dissipated into the hot water.
10 A student heats 84.17 mL of water to 95.27°C using a hot plate. The heated water is added to a calorimeter containing 73.92 mL of cold water. The water temperature in the calorimeter rises from 2.15°C to 37.48°C. The specific heat capacity of water is 4.184 J and the density of water is g. °C 1.00 mL Assuming that heat was transferred from the hot water to the cold water and the calorimeter, determine the heat capacity of the calorimeter. J Heat capacity of calorimeter = °C
8. A sample of ethanol, C₂H5OH, absorbs 23.4 kJ of energy. The temperature of the sample increases from 5.6°C to 19.8°C. What is the moles (n) of ethanol in the sample? The specific heat capacity of ethanol is 2.46 J/g.°C. [3 Moles of ethanol in the sample is:
The table lists the specific heat capacities of select substances. Substance Specific heat capacity (J/g °C) lead 0.128 silver 0.235 copper 0.385 iron 0.449 aluminum 0.903 water 4.184 An unknown substance has a mass of 14.5 g.14.5 g. The temperature of the substance increases by 15.3 ∘C15.3 ∘C when 85.4 J85.4 J of heat is added to the substance.
A 4.70-g sample of aluminum pellets (specific heat capacity = 0.89 J °C- g) and a 10.00-g sample of iron pellets (specific heat capacity = 0.45 J °C- g) are heated to 115.0°C. The mixture of hot iron and aluminum is then dropped into 98.3 g of water at 22.0°C. Calculate the final temperature of the metal and water mixture, assuming no heat loss to the surroundings. The specific heat capacity of water is 4.18 J °C¯'g¬! °C
4. The heat capacity of copper is 0.382 J/g°.C. A 22.6 g sample of copper at 93° C is placed in 50 g of water at 23.9° C. What is the final temperature of the system?
A sample of 175°C copper is placed into a beaker with 100 grams of 25°C water. Which sample of copper will heat the water to the lowest final temperature? The specific heat of copper is 0.385 J-g-1.°C-1. The specific heat of water is 4.184 J·g-1.°C-1. A. 5.0 g Cu B. 2.0 g Cu C. 0.5 g Cu D. 1.0 g Cu
Suppose 2.32 kJ of heat is added to 25.4 g of ethanol at 18.71 °C. The specific heat capacity of ethanolis 2.46 J/g °C. What is the final temperature of the ethanol?